Question

A gas sample containing 0.546 mole collected at 700 mm and 25°C. would occupy what volume?

Answer 1

Answer:

Volume occupied by the gas = 14.511 L

Explanation:

Pressure = 700 mm

The conversion of P(mm) to P(atm) is shown below:

$P(atm)=\frac {1}{760}\times P(atm)$

So,  

Pressure = 700 / 760 atm = 0.921 atm

Temperature = 25 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = 25 + 273.15) K = 298.15 K  

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.921 atm × V = 0.546 mol × 0.0821 L.atm/K.mol × 298.15 K  

⇒V = 14.511 L